The following reaction is first order,
C2H6 → 2 CH3. If the rate constant
is equal to 5.5 × 10-4 s-1 at 1000 K, how
long will it take for 0.35 mol of C2H6 in a
1.00 L container to decrease to 0.15 mol in the same
container?
26 min
6.1 min
71 min
120 min
The following reaction is first order, C2H6 → 2 CH3. If the rate constant is equal...
estion 4 La siguiente reacciones de primer orden, CHE - 2CH. Si la constante de rapidez es igual a 5.5 x 104 1 a 1000 K, cuinto tompo tardarin 0.35 mol de C2He en un contenedor de 1.00L para disminuir a 0.20 mol en el mismo contenedor? The following reaction is first order, CHE -- 2 CH3. If the rate constant is equal to 5.5 x 10- 4 1 at 1000K, how long wil it take for 0.35 mol of...
5. A student is asked to find the rate constant for a first-order reaction, given that (Alo = 10 M and after 20 s the concentration of A is 2.5 M. The student uses the following logic:2 rate = k[A] (for a first-order reaction) So: A[A] – k[A] Δt' Inserting the values gives: (2.5 M - 10 M - 205-05") = k[2.5 M] Solving for k gives 0.15 5-1. a. Do you agree with the student's answer? Why or why...
1) Hydrogen peroxide, H2O2(aq), decomposes to H2O(l) and O2(g) in a reaction that is first order in H2O2 and has a rate constant k = 1.06×10−3 min−1 at a given temperature. How long will it take for 15% of a sample of H2O2 to decompose? 2)The decomposition of nitrogen dioxide, NO2, into nitrogen monoxide and oxygen at a high temperature is second-order in NO2. The rate constant for this reaction is 3.40 L/mol×min. Determine the time needed for the concentration...
The first order reaction of N2O4 to form two mole of NO2 has a rate constant k = 0.023 min–1. How long will it take the initial concentration of N2O4 to decrease to 10 % of the original value? A. 600s B. 43.5s C. 43.5min D. 435 min E. 100 min show working any please
The decomposition of ethane (C2H6) to methyl radicals is a first-order reaction with a rate constant of 5.36 X 10^-4 s ^-1 at 700˚C: C2H6 ---> 2CH3. Calculate the half-life of the reaction in minutes.
The first-order rate constant for the decomposition of
CH3N2CH3,
CH3N2CH3(g) C2H6(g) + N2(g)
at 327 oC is k = 3.60e-04 s-1. Suppose we
start with 0.0505 mol of CH3N2CH3
in a volume of 3.7 L. How many moles of
CH3N2CH3 will remain after
3.76e+01 min?
a) 0.0224 moles will remain.
b) 0.000684 moles will remain.
c) 1.60e-96 moles will remain.
d) 0.0498 moles will remain.
e) 0.0254 moles will remain.
The elementary gas-phase reaction (CH3)3COOC(CH3)3 → C2H6 + 2CH3COCH3 A → B + 2C is carried out isothermally at 400 K in a flow reactor with no pressure drop. The reaction rate constant at 50°C is 10–4 min–1 and the activation energy is 85 kJ/mol. Pure di-tert-butyl peroxide enters the reactor at 10 atm and 127°C and a molar flow rate of 2.5 mol/min, i.e., FA0 = 2.5 mol/min. (d) There appears to be uniform leakage of Ethane through the...
2. Answer the following questions by connecting the half-life of each first-order reaction to the rate constant. a. The rate constant of a first-order reaction is 2.43 × 10–2 min–1. What is the half-life of the reaction? (2 points) b. A first-order reaction has a rate constant of 0.547 min-1. How long will it take a reactant concentration 0.14 M to decrease to 0.07 M? (2 points) c. The half-life of a first-order reaction is 5.47 min. What is the...
first order reaction
First-Order Reactions (35) Azomethane decomposes into nitrogen and ethane at high temperatures according to the following equation: (CH3)2N2(g) — N2(g) + C2H6(g) The following data are obtained in an experiment: Time (h) [(CH3)2N2] 1.00 0.905 2.00 0.741 3.00 0.607 4.00 0.497 (a) By plotting the data, show that the reaction is first-order. (b) From the graph, determine k. (c) Using k, find the time in hours) that it takes decrease the concentration to 0.100 M. (d) Calculate...
The reaction, aA products, is a first order reaction with a rate constant of 1.248 x 10-4 s-1 . a. How long (in seconds) does it take for the initial amount of A to decrease by 30%? b. What fraction of reactant remains after 30 minutes? c. What is the half-life for the reaction? d. How long does it take for the initial amount of reactant to decrease by 87.5%?